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2016-10-24 4:44 pm
In a calorimetry experiment at constant pressure, a student reacts 1.25 g of ZnO (MM=81.38 g/mole) with 40.0 g of aqueous HCl solution to produce aqueous zinc chloride and liquid water. The initial temperature of the solution is 21.72 ⁰C and the final temperature is 23.89 ⁰C. (a) Use the temperature change for the reaction (∆T), the known heat capacity of water (4.184 J/g ⁰C), and the mass of solution to calculate the heat change (q) for the solution. (b) Then calculate the enthalpy change for the reaction occurring in this solution (∆Hreaction) in kJ/mole. Show all of your calculations.

回答 (1)

2016-10-24 5:37 pm
✔ 最佳答案
Heat change of the solution
= m c ΔT
= [(40.0 + 1.25) g] × [4.184 J/(g°C)] × [(23.89 - 21.72)°C]
= +374.5 J

(The positive sign indicates that the solution absorbs heat.)


(b)
Heat change of the solution = -374.5 J
No. of moles of ZnO reacted = (1.25 g) / (81.38 g/mol) = 0.01536 mol

ΔHreaction = (-374.5 J) / (0.01536 mol) = -24400 J/mol = -24.4 kJ/mol


收錄日期: 2021-04-18 15:41:46
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